Question

Sulphuric acid is produced when sulphur dioxide reacts with oxygen and water in the presence of a catalyst: $2S{O}_2\left(g\right)+O_2\left(g\right)+2H_{2}O\left(l\right)\to 2H_{2}S{O}_{4.}$ If $5.6$ mol of $O_2$ and an excess of water is present, the maximum number of moles of $H_{2}S{O}_4$ that can be obtained is :

• A. $2.5$
• B. $2.6$
• C. $10.3$
• D. $11.2$

Answer 1

The correct option is D $11.2$

The balanced reaction is $2S{O}_2\left(g\right)+O_2\left(g\right)+2H_{2}O\left(l\right)\to 2H_{2}S{O}_{4.}$
Assuming excess of sulphur dioxide is present, the amount of sulphuric acid that can be obtained from $5.6$ moles of oxygen is $2\times 5.6=11.2$ moles.